This document discusses the physical and chemical properties of metals. The key physical properties mentioned are high melting points, conductivity of heat and electricity, solid state, and density. The chemical properties discussed are reaction with oxygen to form metal oxides, reaction with water to form hydroxides, reaction with acids to form salts, and displacement reactions where more reactive metals can replace less reactive ones from compounds. Exceptions to some typical metal properties are also outlined, such as the lack of lustre in lead or malleability in mercury.
2. PHYSICAL PROPERTIES
Following are the physical properties of metals:
• high melting points
• good conductors of electricity
• good conductors of heat
• high density
• Solid
• Sonorous
• Lustrous
• Malleable
• Ductile
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3. The property of Metals producing
ringing sound.
Metals are Sonorous
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4. Metals are Lustrous in nature.
They have shiny appearance.
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7. CHEMICAL PROPERTIES
Following are the chemical properties of metals:
• Metals react with oxygen to form metal oxides.
• Metals react with water to form metal hydroxide.
Reactivity with water differs from metal to metal.
• Metals like sodium, potassium, and calcium react
vigorously with dilute HCl and H2SO4 to form their metal
salt and hydrogen.
• Metals that are more reactive will readily with less
reactive metals.
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8. Reaction with Air (Oxygen)
Metals react with oxygen to form metal oxides.
Na+O2 → Na2O (Sodium Oxide)
K+O2 → K2O (Potassium Oxide)
Ca+O2 → CaO (Calcium Oxide)
Mg+O2 → MgO (Magnesium Oxide)
Al+O2 → Al2O3 (Aluminium Oxide)
Metal
Oxides are
Basic in
nature.
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9. Reaction with Air (Oxygen)
Metals react with oxygen to form metal oxides.
• Metal oxides are generally basic in nature but it can
also be amphoteric in nature.
• Amphoteric oxides mean that they are acidic as well
as basic in nature.
• Some metals like sodium and potassium react
vigorously with oxygen.
• Whenever sodium or potassium is exposed to air it
catches fire. Hence, they are kept in kerosene.
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10. Reaction with Water
Metals react with water to form metal hydroxides.
Na+H2O → NaOH+ H2 (Sodium Hydroxide)
K+ H2O → KOH+ H2 (Potassium Hydroxide)
Ca+ H2O → Ca(OH)2+ H2 (Calcium Hydroxide)
Mg+ H2O → MgO+ H2 (Magnesium Oxide)
Fe+ H2O → Fe3O4+ H2 (Iron Oxide) Metal
hydroxides
are Basic
in nature.
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11. Reaction with Water
Some metals react with water to form metal hydroxide whereas
some of them do not react. Reactivity with water differs from
metal to metal.
Metals like Sodium and Potassium are highly reactive. They
react with water to form alkalis such as sodium hydroxide and
potassium hydroxide.
Magnesium and zinc do not react with cold water. They form
their respective oxides when reacted with hot water.
Iron is less reactive than sodium, potassium, calcium, zinc and
magnesium. It does not react with cold and hot water, but it
reacts with steam to form magnetic oxides.
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12. Reaction with Dilute Acids
Metals react with dilute acids to form metal salts with
hydrogen gas.
Mg+ HCl → MgCl2+ H2 (Magnesium Chloride)
Fe+ H2SO4 → FeSO4+ H2 (Iron Sulphate)
Metals like sodium, potassium, lithium and calcium react
vigorously with dilute HCl and H2SO4 to form their metal salt and
hydrogen.
While magnesium, zinc, iron, tin and lead does not react vigorously
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13. Reaction of Metal With Other Metal Salts
Metals that are more reactive will readily react with less
reactive metals.
More reactive metal displaces the less reactive metal from its
oxides, chlorides or sulphides.
Zn + CuSO4 → ZnSO4+ Cu (Zinc Sulphate)
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14. K K
Potassium
Sodium Na Na
Calcium Ca Ca
Magnesium Mg Mg
Aluminium Al Al
Zinc Zn Zn
Iron Fe Fe
Tin Sn Sn
Lead Pb Pb
Copper Cu Cu
Gold Au Au
Silver Ag Ag
Platinum Pt Pt
Decreases
Increases
Displacement reaction is a chemical
reaction in which a more reactive
element displaces a less reactive
element from its compound.
DISPLACEMENT REACTION
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15. EXCEPTIONS
1. Lustrous (Exception: Lead)
2. Hard (Exception: Lithium, Sodium, Potassium)
3. Malleable (Exception: Mercury)
4. Ductile (Exception: Mercury)
5. Good conductor of heat and high melting points
(Exception: Lithium, Sodium, Potassium, Caesium, Gallium)
6. Good conductor of Electricity (Exception: Lead)
7. Sonorous (Exception: Mercury)
8. High Density (Exception: Lithium, Sodium, Potassium)
9. Solids at room temperature (Exception: Mercury).
Gallium becomes a liquid when heated.
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